Campus Units

Document Type

Article

Publication Version

Published Version

Publication Date

12-2003

Journal or Book Title

Journal of the American Chemical Society

Volume

126

Issue

3

First Page

834

Last Page

843

DOI

10.1021/ja0303182

Abstract

Ab initio molecular orbital theory has been used to calculate accurate enthalpies of formation and adiabatic electron affinities or ionization potentials for N3, N3-, N5+, and N5- from total atomization energies. The calculated heats of formation of the gas-phase molecules/ions at 0 K are ΔHf(N3(2Π)) = 109.2, ΔHf(N3-(1∑+)) = 47.4, ΔHf(N5-(1A1‘)) = 62.3, and ΔHf(N5+(1A1)) = 353.3 kcal/mol with an estimated error bar of ±1 kcal/mol. For comparison purposes, the error in the calculated bond energy for N2 is 0.72 kcal/mol. Born−Haber cycle calculations, using estimated lattice energies and the adiabatic ionization potentials of the anions and electron affinities of the cations, enable reliable stability predictions for the hypothetical N5+N3- and N5+N5- salts. The calculations show that neither salt can be stabilized and that both should decompose spontaneously into N3 radicals and N2. This conclusion was experimentally confirmed for the N5+N3- salt by low-temperature metathetical reactions between N5SbF6 and alkali metal azides in different solvents, resulting in violent reactions with spontaneous nitrogen evolution. It is emphasized that one needs to use adiabatic ionization potentials and electron affinities instead of vertical potentials and affinities for salt stability predictions when the formed radicals are not vibrationally stable. This is the case for the N5 radicals where the energy difference between vertical and adiabatic potentials amounts to about 100 kcal/mol per N5.

Comments

This article is from Journal of the American Chemical Society 126 (2003): 834, doi:10.1021/ja0303182.

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